Vanadium(II) chloride

Vanadium(II) chloride
Plan view of a single layer in the crystal structure of vanadium(II) chloride	Layer stacking in the crystal structure of vanadium(II) chloride
Names
	IUPAC name Vanadium(II) chloride
	Other names Vanadous chloride
Identifiers
CAS Number	10580-52-6 ;
3D model (JSmol)	Interactive image;
ChemSpider	59733 ;
ECHA InfoCard	100.031.057
PubChem CID	66355;
RTECS number	YW1575000;
CompTox Dashboard (EPA)	DTXSID60147349 ;
	InChI InChI=1S/2ClH.V/h21H;/q;;+2/p-2 Key: ITAKKORXEUJTBC-UHFFFAOYSA-L ; InChI=1/2ClH.V/h21H;/q;;+2/p-2 Key: ITAKKORXEUJTBC-NUQVWONBAZ;
	SMILES Cl[V]Cl;
Properties
Chemical formula	VCl2
Molar mass	121.847 g/mol
Appearance	pale green solid
Density	3.230 g/cm3
Melting point	1,027 °C (1,881 °F; 1,300 K)
Boiling point	1,506 °C (2,743 °F; 1,779 K)
Solubility in water	soluble
Magnetic susceptibility (χ)	+2410.0·10−6 cm3/mol
Structure
Crystal structure	CdI2
Coordination geometry	octahedral
Hazards
Main hazards	Reacts with oxygen rapidly
R-phrases (outdated)	20/21/22-34
S-phrases (outdated)	26-27-36/37/39-45
Related compounds
Other anions	vanadium(II) fluoride, ; vanadium(II) bromide, ; vanadium(II) iodide
Other cations	titanium(II) chloride, chromium(II) chloride
Related compounds	vanadium(III) chloride
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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	Infobox references

Vanadium(II) chloride is the inorganic compound with the formula VCl₂, and is the most reduced vanadium chloride. Vanadium(II) chloride is an apple-green solid that dissolves in water to give purple solutions.[1]

Preparation, properties, and related compounds

Solid VCl₂ is prepared by thermal decomposition of VCl₃, which leaves a residue of VCl₂:[1]

2 VCl₃ → VCl₂ + VCl₄

VCl₂ dissolves in water to give the purple hexaaquo ion [V(H₂O)₆]²⁺. Evaporation of such solutions produces crystals of [V(H₂O)₆]Cl₂.[2]

Structure

Solid VCl₂ adopts the cadmium iodide structure, featuring octahedral coordination geometry. VBr₂ and VI₂ are structurally and chemically similar to the dichloride. All have the d³ configuration, with a quartet ground state, akin to Cr(III).[3]

Vanadium dichloride is a powerful reducing species, being able to convert sulfoxides to sulfides, organic azides to amines, as well as reductively coupling some alkyl halides.

References

Young, R. C.; Smith, M. E. "Vanadium(II) Chloride" Inorganic Syntheses, 1953, volume IV, page 126-127.doi:10.1002/9780470132357.ch42
Martin Pomerantz, Gerald L. Combs, N. L. Dassanayake, "Vanadium Dichloride Solution" Inorganic Syntheses, 1982, vol. XXI, pp. 185–187. doi:10.1002/9780470132524.ch42
Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.

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[IS-1] Young, R. C.; Smith, M. E. "Vanadium(II) Chloride" Inorganic Syntheses, 1953, volume IV, page 126-127.doi:10.1002/9780470132357.ch42

[2] Martin Pomerantz, Gerald L. Combs, N. L. Dassanayake, "Vanadium Dichloride Solution" Inorganic Syntheses, 1982, vol. XXI, pp. 185–187. doi:10.1002/9780470132524.ch42

[3] Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.